CHEM 201 - 11.26.07

CHEM 201 - 11.26.07 - o Gases 1 atm Solutions 1M...

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CHEM 201 – November 26, 2007 A + B  C + D Rates o Rate Forward = k f [A][B] o Rate Reverse = k r [C][D] 1/k r = [C][D] k c = [C][D]/[A][B] = k f /k r Electrochemistry o Zn (s) + Cu 2+ (aq) Zn 2+ (aq) + Cu (s) wire salt bridge metal strips are in a SO 4 solution Cu Zn Reduction – cathode Oxidation – anode Definitions o Electrodes - Metal strips connected with wire o Salt bridge – u-shaped tube filled with inert electrolyte gel o Anode – where oxidation takes place (AO vowels) o Cathode – where reduction takes place (CR consonants) Drawing convention o Anode half cell drawn on the left with a double line (||) and the cathode half cell on the right The double line represents the salt bridge o Electrode | Anode Solution || Cathode Solution | Electrode Zn (s) | Zn 2+ || Cu 2+ | Cu (s) o Electrons always flow from anode to cathode Standard Conditions
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Unformatted text preview: o Gases @ 1 atm Solutions @ 1M Temperature @ 25°C o Standard Potential is under conditions (E ) Not standard (E) Galvanic Cell/Voltaic Cell o E cell = E reduction + E oxidation o E oxidation = – E reduction o E cell = E reduction of the cathode – E reduction of the anode Standard Half-cell potential is the difference in voltage between an electrode and a standard electrode o Standard Hydrogen Electrode (SHE) Platinum electrode in contact with H 2 and H + SHE ≡ 0 V If not given an equation, the more positive E red value is the cathode o Cu 2+ + 2e- Cu E = 0.34V Zn Zn 2+ + 2e-E = 0.76V E cell = 1.10 V New Example o Silver-Zinc o Zn (s) | Zn 2+ ||Ag + |Ag (s)...
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CHEM 201 - 11.26.07 - o Gases 1 atm Solutions 1M...

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